For the reaction at 20 degree C, the equilibrium constant is calculated to be K

Question

For the reaction at 20 degree C, the equilibrium constant is calculated to be K = 4.5 times 10^8. Write the equilibrium expression for this reaction. From the size of the number for K, does the equilibrium lie to the left or to the right? If a base (NaOH) was added to the mixture, in which direction would the reaction shift, to the left or to the right? Explain your answer. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? Show your work. In the reaction below, the equilibrium constant is 10^-34. Is this reaction likely to take place? Explain your answer.

Explanation / Answer

Q1-

K = 4.5*10^8

a)

K = [products]/[reactants]

K = [NH4+]/ ([NH3][H+])

b)

since K >> 1, this must favour products

K = [NH4+]/ ([NH3][H+]) >> 1, that is, NH4+ formation or to the right

c)

if NaOH is added, then OH- ions are rich in solution, those react with H+ to form H2O

then the reagents decrease, therefore equilibrium shisfts toward left

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